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Determine the equilibrium pH of aqueous solutions for the following strong acids

  1. Sep 26, 2012 #1
    Determine the equilibrium pH of aqueous solutions for the following strong acids or bases: (a) 257mg/L of HSO4- ; (b) 10nM NaOH ; (c) 75ug/L of HNO3
     
  2. jcsd
  3. Sep 27, 2012 #2

    AGNuke

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    Gold Member

    Look for their respective Ka values on net.
     
  4. Sep 27, 2012 #3
    I kind of figured it out except for the first one, because HSO4- can become an acid or a base depending what it's mixed with so I don't know what to do, do I get the pH or the pOH? And how?
     
  5. Sep 27, 2012 #4

    Borek

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    Staff: Mentor

  6. Sep 27, 2012 #5
    Thanks
     
  7. Sep 27, 2012 #6
    Not totally relevant to the OP, but part (b) of this exercise is nonsensical in any practical terms. I bring this up because we are in the "Chemistry" forum rather than the "Chemistry Homework" forum.

    The answer to a formal calculation to part (b) will only bear any relationship to reality if the concentration of carbon dioxide/bicarbonate in the water is much smaller than that of the hydroxyl -- say 1 nM or less. Any normal aqueous solution will be acting as a carbonate buffer for such low levels of hydroxyl, and I would like to know how anyone proposes to prepare a water sample that is accessible for normal laboratory work, but less than 1 nM in bicarbonate/carbon dioxide.
     
  8. Sep 27, 2012 #7

    Borek

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    Staff: Mentor

    It is a typical trick question asked every year :smile:

    And heck, you are right about homework... Moving the thread.

    toby: please read forum rules.
     
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